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Chapter 8: Q56P (page 369)

What orbital do the lone-pair electrons occupy in each of the following compounds?

Short Answer

Expert verified

a) Nitrogen is attached with carbon with a single bond hence it is sp3hybridized.

b) Nitrogen is attached with carbon with a double bond hence it is sp2hybridized.

c) Nitrogen is attached with carbon with a triple bond hence it is sphybridized.

Step by step solution

01

How we determine this

a) Nitrogen is attached with carbon with a single bond hence it is sp3hybridized.

b) Nitrogen is attached with carbon with a double bond hence it is sp2hybridized.

c) Nitrogen is attached with carbon with a triple bond hence it is sphybridized.

02

Final answer

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Most popular questions from this chapter

Which species in each pair is more stable?

a. When HBr adds to a conjugated diene, what is the rate-determining step?

b. When HBr adds to a conjugated diene, what is the product-determining step?

Which loses a proton more readily: a methyl group bonded to cyclohexane or a methyl group bonded to benzene?

Which of the following are aromatic?

The acid dissociation constant (Ka) for loss of a proton from cyclohexanol is 1 脳10-16.

a. Draw a reaction coordinate diagram for loss of a proton from cyclohexanol.

b. Draw the resonance contributors for phenol.

c. Draw the resonance contributors for the phenolate ion.

d. On the same plot with the energy diagram for loss of a proton from cyclohexanol, draw an energy diagram for loss of a proton from phenol.

e. Which has a greater Ka: cyclohexanol or phenol?

f. Which is a stronger acid: cyclohexanol or phenol?
See all solutions

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